Ideal Gas Law solve for partial pressure

[Jef123]

1. Gaseous compound Q contains only xenon and oxygen. When 0.100 g of Q is placed in a 50.0 mL steel vessel at 0 °C, the pressure is 0.229 atm. When the vessel and its contents are warmed to 100 °C, Q decomposes into its constituent elements. What is the total pressure, and what are the partial pressures of xenon and oxygen in the container?



2. Molecular formula = XeO₄



3. I used the ideal gas law formula PV = nRT. I know that the moles (n), gas constant (R), and volume (V) are constant, so I can solve for the new pressure using the equation P₁/T₁= P₂/T₂. Rearranging to solve for P₂ = 0.313 atm

Apparently 0.313 atm is the partial pressure for Xenon and 0.626 atm is the partial pressure for oxygen. I know that when the temperature is increased that the compound breaks into its constituent elements (i.e. Xe and 2O₂) but what I do not understand is why would the equation I used to solve for pressure give me the partial pressure of xenon? I thought that 0.313 atm would be the total pressure of both gases in the vessel?

 

[Chestermiller]

How did the total number of moles of gas in the vessel change when the compound decomposed? How many moles of X were formed, and how many moles of O2 were formed?

Chet

 

[Jef123]

Oh, so two moles of O2 were formed and 1 mole of Xe were formed. So i just needed to multiply the amount of moles by 2 to solve for O2. Thanks!